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Sodium paraperiodate arrived on the scene as oxidation chemistry kept finding new puzzles to solve. Early chemists hunting for reliable ways to break apart organic molecules saw the promise in periodate salts, and sodium paraperiodate quickly stood out for its selectivity and stability. Through the twentieth century, researchers tinkered with its structure, stashing it next to sodium metaperiodate and other oxidizers to pick from according to reaction needs. This salt has become a standard reagent on lab benches, its path marked by patent filings, improvements in synthesis, and broader uses in both organic and inorganic labs. Chemical suppliers picked up on academic demand and packaged it for ready use, cementing its status as a tool for controlled oxidation. In both university research and industrial process development, the reagent has helped develop assays, enable analytical work, and create new functional groups for bigger, more complicated molecules. Over decades, folks working on synthetic routes or enzyme chemistry often mention their first encounters with sodium paraperiodate—usually during tough reaction optimization projects where other oxidizers proved too blunt or too rough on targets needing a gentler hand.
Sodium paraperiodate emerges as a white, crystalline solid, relatively easy to store. Its formula, Na5IO6, points to the high oxidation state of iodine, something seasoned chemists see as an advantage for cleaving specific bonds, like the vicinal diols in carbohydrates. Commercial products usually arrive in sealed containers since moisture or environmental contaminants can nudge the material toward unwanted changes. The substance fits well in any kit meant for selective oxidation, especially in labs focused on carbohydrate sequencing, glycoprotein modification, or sensitive organic syntheses. For research and pilot production, material comes in multi-gram or larger batches, often supported by detailed documentation on batch history, purity, and moisture content. A surprising number of small labs rely on consistent grades from different suppliers because even a small variance often means tricky downstream purification. Research discussion threads carry plenty of tales about how switching to a new bottle or changing lots led to vastly different oxidation efficiency or reaction color—common headaches for anyone chasing reproducibility.
Sodium paraperiodate carries a molecular weight close to 387 g/mol. Its crystals sit stably at room temperature, and handling feels not much different from other inorganic salts, though their sharp edges dust easily when scooped. The salt dissolves well in water, which suits it for most reaction setups aiming at aqueous environments. On contact with moisture, sodium paraperiodate breaks down slowly, shifting color from brilliant white to faintly yellow as iodine species shuffle about. The chemical shows a strong oxidizing character, pouncing on vicinal diols to break apart the carbon backbone with surgical precision while leaving other bonds mostly untouched. Heat doesn’t do it favors, either; store it cool and dry because elevated temperature can trigger unwanted degradation, liberating iodine and erasing the carefully controlled oxidation potential. Chemists who have relied on it in tough oxidations rarely forget its smell—a faint hint of ozone paired with that metallic tang—reminding them of its reactive personality.
Purchasing sodium paraperiodate means sifting through technical bulletins to pick the right grade. The purity often lands beyond 98%, with documentation spelling out water content, limits for heavy-metal impurities, and exact iodine content per mole. Suppliers stamp hazard labels for oxidizer risk and the corrosiveness that comes with mixing into water. Storage recommendations lean heavily on keeping containers tightly sealed, in non-reactive environments, with clear warning icons and emergency handling guides. Anyone ordering by mail faces several layers of compliance paperwork since oxidizers trigger regulatory oversight—shipping teams pay special attention to temperature conditions during transit. In regulated pharmaceutical or food labs, sodium paraperiodate’s lot documentation and traceability become a bigger deal, tracked down to storage date, handling personnel, and disposal logs. This level of detail helps labs respond to audits and trace any anomaly back to a particular lot or handling period, invaluable for complying with quality standards.
The main route to sodium paraperiodate combines sodium hydroxide and periodic acid under tight control of pH, temperature, and mixing rate. The result is slow crystallization as the sodium and iodine species reorganize in solution, locking water molecules into the lattice based on conditions set during reaction and drying. Some industrial-scale makers employ continuous-flow reactors to manage heat and control yield while suppressing side products that sap overall efficiency. Filtration and washing routines strip away unreacted sodium hydroxide and leftover acid. Crystallization takes hours, sometimes a day, followed by vacuum drying to drag out any stubborn water hiding in the crystal pockets. Labs making their own often recycle excess periodic acid, a practice that cuts cost and limits waste streams, especially in facilities where sustainability and waste reduction sit high on the operative agenda. The resulting solid needs careful packaging—any sloppiness in this last step risks introducing acids, dust, or other contaminants that hamper downstream performance.
Sodium paraperiodate’s star reaction remains its clean cleavage of vic-diols, splitting the carbon-carbon bond down the middle and forming two aldehyde groups—a reaction that scientists rely on for mapping out sugar structures or modifying polymers that need site-selective functionalization. It leaves most other functional groups untouched, a feat not matched by bulkier or less selective oxidizers. The product’s use expands still further in bioconjugation, opening up new binding sites in biomolecules or prepping samples for proteomics and glycomics. It also helps create precursors for more complex organic syntheses, delivering target fragments with minimal over-oxidation or side reactions. Advanced research groups sometimes tweak the salt itself, exploring mixed salts that tune reactivity or solubility for niche applications. Person-to-person notes often mention mixing with buffer salts, adjusting pH to fine-tune the oxidation without wrecking sensitive targets. Some labs keep detailed logs on each reaction batch—monitoring color shifts or gas evolution as signposts of progressing chemistry—since subtle variations can derail a long line of syntheses or analysis steps if left unchecked.
Sodium paraperiodate goes by a few other names, making it a regular item on multiple chemical catalogs and databases. You’ll spot it labeled as sodium periodate, sodium orthoperiodate, and the sodium salt of periodic acid. Sometimes, chemical shorthand like Na5IO6 pops up in reaction schemes, especially where space is tight or notation needs to match legacy literature. Whether browsing catalog numbers or reading old papers, chemists swap stories about chasing down the exact variant needed, as even a small shift in composition changes outcomes. Vendors sometimes cross-list product codes to clear up confusion, though experienced scientists learn to double-check the fine print. For less experienced users, those small nuances in name can spell headaches—ordering the wrong type leads to delays, wasted time, and frustrated students looking to their mentors for clarity in the quirks of chemical naming.
Safety with sodium paraperiodate means more than gloves and aprons. The substance reacts fast not just in target reactions but if it meets the wrong mix of organic material or reducing agents. In practice, trained staff pay close attention to both storage and handling, keeping it away from flammables and stashing smaller quantities in desiccated cabinets or explosion-rated lockers. Local exhaust hoods or ventilated enclosures become necessary because fine dust irritates the lungs and oxidizer dust floats up quickly from scoops or weighing boats. Eye wash stations and neutralizing spills feature in standard operating protocols. Disposal rules stop users from mixing waste with general trash; specialty bins and licensed waste handlers handle spent reagents and anything contaminated. Anyone ordering the solid for the first time usually takes a safety refresher, because even minor spills can rapidly escalate, especially if mixed with other bench reagents. This attention to detail on safety routines keeps small accidents from scaling up into bigger incidents.
Applications for sodium paraperiodate cluster in carbohydrate chemistry, but the real reach stretches into proteomics, environmental analysis, materials research, and diagnostics. Analysts leverage the oxidizer’s selectivity to open up sugar rings or create handles for further modification—work crucial in sequencing sugars from biological samples or designing antibody-drug conjugates. In environmental labs, sodium paraperiodate clears up phenol residues or complex organic pollutants, breaking them down into more manageable fragments before measurement. Material scientists run tests to tweak conductivity or chemical affinity in polymer blends by site-selective modification, a task sped up by the periodate’s specificity and gentle reaction speed. For protein chemists, attaching new labels onto glycosylated amino acids depends on the clean break offered during diol cleavage. Diagnostic kit makers prize the compound’s ability to boost assay accuracy—the aldehyde groups introduced raise signal strength or yield sharper contrast. Hearing from colleagues who spend long days tweaking reaction conditions, the comment usually comes down to trust: sodium paraperiodate delivers where broad-spectrum or less predictable oxidizers tend to fumble.
Research investments keep delivering new applications for sodium paraperiodate. Groups at universities dabble in hybrid catalysts, embedding the salt into polymer matrices or nanomaterial scaffolds. Others examine the salt’s efficacy in microfluidic systems, shrinking reaction footprints while keeping efficiency high. Drug discovery circles see regular use in mapping out glycosylation patterns, supporting the search for new therapeutics or vaccine targets. Each year, papers and patents add twists to preparation, sometimes enhancing reactivity through dopants or alternately slowing down the reaction for ultra-selective processes. Multicenter collaborations examine next-gen application in environmental cleanup or precise organic synthesis, sharing open-access methods for green chemistry protocols that minimize byproduct formation and simplify downstream separation. Private industry pushes to develop new labeling reagents, diagnostics, and polymers using sodium paraperiodate’s reliable chemistry as a launching point. Personal stories from these projects often highlight how troubleshooting and iterative testing—tuning batch concentration, modifying crystal habits, or exchanging buffer salts—finally yield the right tool for everyday lab challenges.
Toxicity assessment forms a regular part of sodium paraperiodate research. Acute exposure to dust or concentrated solutions causes irritation to skin, eyes, and the respiratory tract, leading health and safety officers to classify it firmly under hazardous materials. Studies report oxidative stress in tissue samples and cultured cells, indicating the salt’s reactivity is not just limited to the test tube. Chronic environmental effects have drawn less attention, but environmental agencies flag it as a potential pollutant if it enters water streams at scale. Chemists tasked with disposal plan procedures that quench or reduce the oxidizer, often running reaction mixtures with reducing agents before waste handling. In the course of animal testing, sodium paraperiodate exhibits marked toxicity, with dose-dependent effects that call for strict containment and well-documented handling logs. Lab managers who have handled incidents note that quick identification—coupled with fast first aid and immediate decontamination—stemmed escalation and limited health impacts in exposed staff.
The future for sodium paraperiodate points to smarter applications and greener operational models. Advanced research previews hybrid applications—integrating periodate chemistry with modern microfabrication, materials design, or digital sensing technology. Academic and industry collaborations probe ways to recycle or regenerate used salt or adapt the chemistry to low-waste settings that mesh better with circular-economy principles. Regulatory bodies push for less reliance on hazardous oxidizers, yet smart engineering and clever chemistry keep sodium paraperiodate on the roster through improved handling, recovery, and safer packaging methods. In pharmaceutical research, demands for sharper glycan analysis and high-performance drug conjugation only heighten dependence on this reliable reagent. Innovation now hinges on reducing exposure risk, lowering environmental impact, and integrating digital tracking for complete life-cycle management. For anyone used to juggling research, regulatory compliance, and operational safety, sodium paraperiodate keeps offering new questions, technical puzzles, and opportunities for meaningful scientific advances across sectors.
Sodium paraperiodate’s name sounds like something from a chemistry textbook that most people would rather avoid. But this white, crystalline powder has a job in more corners of life than most realize. In my time working alongside folks in labs and manufacturing, sodium paraperiodate came up in conversations mixed with a bit of caution and a lot of respect.
This chemical belongs to a group of strong oxidizers. That means it’s a powerhouse for snatching electrons from other molecules. Think of it as a cleanup crew for unwanted “junk” floating around in certain materials. In day-to-day terms, it helps break things apart at a molecular level. That sounds technical, but the real-life value is clear once you see where it shows up.
Lab analysts use sodium paraperiodate because it clears out unwanted sugars in complex samples. Let’s say someone’s studying glycoproteins—those odd proteins with sugar chains dangling from them. This chemical strips away the sugars without tearing up the protein itself. That precise work helps develop newer, targeted medicines. Researchers fine-tune insulin treatments and vaccines using steps that often involve sodium paraperiodate.
Environmental testing labs lean on this chemical, too. It breaks down contaminants in soil and water samples, making it easier to spot hidden toxins. If you value clean water and air, then you already depend on the behind-the-scenes work that sodium paraperiodate enables.
Electronics manufacturing can’t run without good cleaning agents. Circuit boards and microchips collect more grime than folks realize. Sodium paraperiodate cleans away leftover organics during the production process. Cleaner surfaces mean more reliable gadgets—phones, computers, and medical devices among them. That matters when you consider how quickly dirty components lead to breakdowns.
This chemical steps up for paper makers, too. It’s used in the bleaching process, helping turn wood pulp from a dingy brown to the bright white most businesses want. While there’s controversy over chemical use in manufacturing, I’ve watched crews balance safety and final product demands carefully, especially with such strong substances.
Every chemist learns early: strong oxidizers deserve respect, not casual handling. Labels with sodium paraperiodate remind workers to keep it away from organic materials or anything that might catch fire. Most factories store it under strict rules, and good training means fewer accidents. Stories from older plant workers about prior mishaps hammered home just how serious safety guidelines are. That level of rigor fits well with what health organizations like OSHA or CDC recommend.
Many manufacturers and research labs now search for alternatives that lower environmental impact or reduce health risks. Green chemistry principles drive new research, focusing on methods that ditch harsh chemicals when possible. Some research groups investigate how to recycle sodium paraperiodate or capture its waste safely—a move that saves money and keeps communities healthier.
Sodium paraperiodate isn’t something people think about unless their job puts it in their hands, but its reach spans clean tech, health, and daily goods. The real challenge stays the same: get the benefits, manage the risk, and keep looking for safer, cleaner ways to solve the same problems.
Sodium paraperiodate holds a spot on any chemist’s shelf who deals with organic synthesis or analytical testing. The formula for this compound looks simple on paper, yet it signals a lot about how the substance works. You’ll find it written as Na5IO6, with five sodium atoms, one iodine, and six oxygen atoms per molecule. That balance tells its own story—less about some textbook example and more about how elements combine to create chemicals that serve people in labs around the world.
In practice, sodium paraperiodate’s ability to oxidize other molecules shapes its usefulness. You can find this compound in reactions that need to break down complex carbohydrates or prepare samples for further analysis. Its strong oxidizing power lets it cleave vicinal diols—think about that in context of sugar chemistry, or even molecular biology, where breaking targeted bonds means everything.
From my experience in a teaching lab, getting a clean reaction sometimes feels impossible, but sodium paraperiodate steps in and delivers crisp results. You watch stubborn compounds split, releasing products you can track and measure. Medical diagnostics, food safety, and research labs don’t just see Na5IO6 as a formula—they see a reliable coworker.
You won’t find this chemical used carelessly. The compound’s strength means those oxygen atoms, so eager to react, can also bring risk. Keeping sodium paraperiodate dry and away from organic materials gets drilled into every lab worker. Oxidizers shouldn’t mix with flammable substances, and this one stays true to form. Gloves, goggles, and well-ventilated spaces aren’t just suggestions—they are the baseline. Breathing dust from this stuff or letting it touch skin would mean a bad day for anyone.
Reports from workplace incidents remind us: even pros get hurt when rushing or cutting corners. Reliable storage keeps the lab running safely. Manufacturers label packaging clearly, and experienced hands keep extra stock secured, ready to meet a chemistry challenge without raising risk.
Industries producing chemicals with strong oxidizers like sodium paraperiodate must think beyond making a sale. I’ve seen environmental compliance become part of the production line. Handling the waste after using Na5IO6 involves chemical neutralization and testing water that leaves a facility. Regulatory standards now ask companies to track their waste streams. Those requirements don’t just tick boxes—they push chemists and manufacturers toward new solutions, often with greener chemistry in mind.
Laboratory-scale use still makes a blip compared to industrial quantities. Yet even a single spill needs proper cleanup. Training labs with up-to-date spill kits and having smart chemical management policies helps everyone in the building. More companies are pushing research into alternate oxidizers or finding closed-loop systems that capture and reuse reagents, reducing waste as much as possible.
Sodium paraperiodate, with its clear formula Na5IO6, serves more than just academic curiosity. Its power in the lab supports real progress. Strong safety practices, reliable sourcing, and environmental awareness set the tone for responsible chemistry. Learning about and respecting this compound ensures cleaner results and safer workspaces, whether I’m teaching students about reactions or talking with industry partners about production flows. Chemistry keeps moving forward, one well-chosen reagent at a time.
Sodium paraperiodate shows up in many labs, from chemical research to forensic investigations. As someone who has spent years surrounded by shelves stacked with glassware, bottles, and chemicals, a few basics always come up for debate: how to keep things safe and how to keep things pure. With sodium paraperiodate, it's not only about ticking boxes for safety audits—it’s about protecting health, data integrity, and expensive equipment.
Sodium paraperiodate breaks down quickly if it absorbs moisture from the air or gets too warm. On contact with organic materials, it acts as a strong oxidizer. Stories circulate about bottles foaming over or corroded caps giving out, all thanks to a bit of neglect or a mislabeled shelf. Besides wasting money, these events risk much worse outcomes, including chemical burns and ruined experiments.
Locking sodium paraperiodate away in a cool, dry place is the plainest defense. Ordinary metal cabinets just won’t cut it, as even a slow trickle of humidity invites lumps and stale product. Many seasoned chemists stick with desiccators or air-tight, labeled containers, often with silica gel packs tucked inside. This stems from firsthand experience—moisture spoils a batch long before anyone sees caked powder or clumps at the bottom of the jar.
Any time oxidizers get stored near flammable organics, solvents, or acids, the risk jumps. During my time in university labs, mixing storage wasn’t just a rule violation; it spelled dangerous accidents. One fire involved nothing more than a cracked cap and a forgotten plastic container nearby. Hydrogen peroxide and sodium paraperiodate, kept together for convenience, ended up wrecking an entire storage unit. Painful lessons meant bringing back frequent risk reviews and committed, clear labeling of everything from the smallest vial to the largest drum.
Every label should announce hazards and include the right hazard pictograms. All staff—not just the most experienced—need to know what each bottle contains and what it does. A distracted intern once grabbed the wrong white powder during a synthesis run. Split-second confusion led to cleanup headaches and delayed results. This sort of mix-up proves that clear, permanent markers are worth their weight in gold.
In multi-use facilities, separate shelves or locked cabinets often solve the problem of unauthorized access. Facilities that take security a notch up with key card access or CCTV see far fewer accidents. This isn’t paranoia—it’s knowledge from long nights cleaning up preventable messes.
Closed containers stop most vapors, but storage rooms still need good airflow. No one wants a garage or supply room filled with escaping fumes, so exhaust systems and humidity gauges become day-to-day tools. Some labs assign a senior member to inspect storage areas at the start of each week. This habit helped spot an unnoticed water leak in a poorly sealed storeroom—dodging both wasted supplies and the potential for a dangerous chain reaction.
Ordering in bulk makes financial sense but backfires if you don’t track every gram. I’ve seen chemicals expire or degrade because they sat unused in a dark corner. Smart labs keep logs to monitor how much comes in, who touches what, and when things reach expiration. Some invest in digital inventory software, helping the team catch problems early and stop over-ordering.
It’s not about overkill—it’s about keeping the people and results safe. Sodium paraperiodate rewards simple, committed care. Each step means fewer surprises, cleaner science, and safer workdays.
Sodium paraperiodate crops up in chemical labs, especially in analytical chemistry and organic synthesis. It plays the role of an oxidizing agent. Scientists use this compound when breaking down complex molecules or spotting small sugar groups in biochemistry. Its use extends to industries that work with dyes or paper, mainly because it helps strip away stubborn substances.
Few people outside of a lab recognize sodium paraperiodate, but anyone handling it knows it isn’t friendly. It carries strong oxidizing properties, and that presents real danger. Direct contact spells trouble for skin and eyes, causing burns or serious irritation. Breathing in its dust stings the nose, throat, and lungs, leading to coughing and possible breathing difficulties. The compound doesn’t need huge amounts to trigger a reaction—a tiny cloud can be enough to set off symptoms, especially in poorly ventilated spaces.
Researchers studying similar oxidizing salts have seen cases where repeated exposure damages mucous membranes and even sensitive tissues in the respiratory tract. In some situations, accidental skin exposure has led to dermatitis or delayed healing. Evidence from occupational safety data highlights the importance of gloves, face shields, and excellent ventilation every time sodium paraperiodate leaves its container.
Sodium paraperiodate enters water supplies through spills. There’s concern for aquatic life. Small invertebrates and fish deal badly with oxidative chemicals and may not recover. Even trace levels risk disrupting a delicate ecosystem. Environmental agencies encourage strict waste handling, since the effects on water don't reverse overnight. Soil organisms feel the impact, too, as sodium paraperiodate breaks down some compounds that plants depend on. That means any leak can ripple through the food chain. This compound demands careful handling all through its lifecycle, from purchase to final disposal.
Jobs requiring sodium paraperiodate often draw people with careful training. Safety data sheets from major suppliers mark it as hazardous. Laboratories stock emergency eyewash stations nearby and train staff to deal with accidental spills. Government bodies and the Occupational Safety and Health Administration urge anyone working with sodium paraperiodate to wear full protective gear, run fume hoods, and store the chemical away from flammable materials. Mixing it with organic matter, acids, or reducing agents could trigger violent reactions. The local fire department treats it as a possible explosion hazard in case of a fire—oxidizers make flames burn hotter and faster.
One fix involves keeping amounts as small as possible, only using it when the project really calls for it. Quality training stands out as another answer—workers familiar with the dangers see fewer injuries and accidents. Lab managers need to run regular reviews of their storage and waste routines, double-checking that nothing leaks and no one forgets the rules. Anyone pouring or handling sodium paraperiodate should have direct guidance on what to do if exposure happens, including the quickest route to medical help.
Chemists continue to hunt for safer oxidizers. Green chemistry pushes for less toxic or easier-to-neutralize chemicals. Some labs swap out sodium paraperiodate for milder, less hazardous compounds when possible, shrinking the health and environmental footprint. Switching makes sense where the risk outweighs the reward, or if safer substitutes deliver the same results.
Sources:Walking through a typical university chemistry building, the heavy glass bottles of sodium paraperiodate usually capture my attention. In research, this chemical plays a hands-on role in breaking down complex organic molecules. It cuts carbon–carbon bonds next to certain functional groups, helping scientists map out molecule structures and synthesize new compounds with precision.
One striking use appears in carbohydrate chemistry. Sodium paraperiodate allows researchers to cleave sugar rings cleanly at specific points, making it easier to modify or study carbohydrates. For example, scientists dissect glycoproteins with this reagent, helping to unravel the role sugars play in diseases or immune responses.
Sodium paraperiodate pulls its weight beyond the basic lab bench by enabling advanced medical diagnostics. Histologists rely on it to prepare tissue samples for detecting diseases, giving clear results by highlighting certain carbohydrates, like in periodic acid-Schiff (PAS) staining. Any lab technician who has processed a biopsy likely recognizes the importance of this reagent in accurate diagnosis.
Researchers developing biosensors have also tapped into the chemical’s oxidative clout. By tweaking surface carbohydrates on sensor chips, they stick biomolecules precisely onto these platforms, creating new ways to test for viral particles or metabolic disorders in tiny blood samples.
The textile industry, usually associated with color and fibers, benefits from sodium paraperiodate’s ability to modify natural polymers. Cotton and other plant-fiber-based textiles can be treated to alter their structure, improving their performance or dyeability. Chemists apply the compound to break down structure just enough to let in functional dyes or inks—making prints more durable or allowing textiles to serve technical roles, from filtration to electronics.
In polymer chemistry, the chemical transforms starches and celluloses. By tailoring their molecular structure, companies give their products new strengths, improved absorbency, or specialized bonding for coatings and adhesives. This chemistry underpins everyday products like medical gauzes and specialty papers.
Using powerful chemicals demands real responsibility. Sodium paraperiodate’s strong oxidative properties mean spills or careless disposal carry health and environmental risks. Training lab staff and setting up secure waste collection go hand-in-hand with its use in research and manufacturing.
Switching to greener alternatives poses a challenge. No drop-in replacement matches its effectiveness in all applications, though research teams keep searching for solutions that balance safety and performance. Some switch to less hazardous reagents for teaching labs or routine procedures, saving sodium paraperiodate for tasks where no substitute delivers required results.
Supporting high-quality research and industrial progress means understanding both the power and the pitfalls of chemicals like sodium paraperiodate. Scientists and engineers must weigh benefits against risk, designing procedures that minimize exposure and waste. Sharing knowledge on safer handling practices, especially for new graduate students or factory technicians, keeps standards up and incidents down.
Future improvements likely rest on developing new catalysts or engineered enzymes to target the same molecular bonds. For now, sodium paraperiodate remains a staple in labs and factories wanting sharp, reliable results in carbohydrate work and material modification.
| Names | |
| Preferred IUPAC name | disodium tetraoxidodioxidosulfate(2−) |
| Other names |
Sodium metaperiodate Sodium periodate Disodium periodate |
| Pronunciation | /ˌsoʊdiəm ˌpærəpɪˈrɪədeɪt/ |
| Identifiers | |
| CAS Number | 7790-28-5 |
| Beilstein Reference | Beilstein Reference: 3944006 |
| ChEBI | CHEBI:66144 |
| ChEMBL | CHEMBL135108 |
| ChemSpider | 20045084 |
| DrugBank | DB11054 |
| ECHA InfoCard | 100.028.864 |
| EC Number | 232-197-6 |
| Gmelin Reference | 132145 |
| KEGG | C18608 |
| MeSH | D011183 |
| PubChem CID | 24861855 |
| RTECS number | SD7200000 |
| UNII | X6L3K2M71N |
| UN number | UN1479 |
| CompTox Dashboard (EPA) | QCAT000240 |
| Properties | |
| Chemical formula | NaIO4 |
| Molar mass | 245.89 g/mol |
| Appearance | White crystalline powder |
| Odor | Odorless |
| Density | 3.865 g/cm³ |
| Solubility in water | soluble |
| log P | -13.5 |
| Vapor pressure | Negligible |
| Acidity (pKa) | ~3.29 |
| Basicity (pKb) | 10.25 |
| Magnetic susceptibility (χ) | -51.0e-6 cm³/mol |
| Refractive index (nD) | 1.60 |
| Viscosity | 15 mPa.s (20 °C) |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 176 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | −734.1 kJ·mol⁻¹ |
| Pharmacology | |
| ATC code | S01XA51 |
| Hazards | |
| Main hazards | Oxidizer, harmful if swallowed, causes eye and skin irritation |
| GHS labelling | GHS05, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Danger |
| Hazard statements | Hazard statements: H272, H302, H318 |
| Precautionary statements | P210, P220, P221, P280, P370+P378, P305+P351+P338, P310 |
| NFPA 704 (fire diamond) | 3-0-1-OX |
| Lethal dose or concentration | LD50 oral rat 3,617 mg/kg |
| LD50 (median dose) | LD50 (median dose): Mouse oral 960 mg/kg |
| PEL (Permissible) | Not established |
| REL (Recommended) | 25°C |
| IDLH (Immediate danger) | IDLH: Not listed |
| Related compounds | |
| Related compounds |
Sodium metaperiodate Periodic acid Potassium periodate Sodium iodate Sodium hypoiodite |
